Question

a five litre flask contains 3.5 gm of N2,3g of H2 and 8g of O2 at 27 celcius the total pressure extracted by the mixture and partial pressure of oxygen is​

Answer 1

Hey Dear,

◆ Answer -

Total pressure = 9.35×10^5 Pa

Partil pressure of oxygen = 1.24×10^5 Pa

● Explanation -

Moles of N2 -

n(N2) = 3.5 / 28

n(N2) = 0.125 mol

Moles of H2 -

n(H2) = 3 / 2

n(H2) = 1.5 mol

Moles of O2 -

n(O2) = 8 / 32

n(O2) = 0.25 mol

Total no of moles of gases -

n = 0.125 + 1.5 + 0.25

n = 1.875 mol

To calculate total pressure,

PV = nRT

P = nRT / V

P = 1.875 × 8.314 × 300 / 5×10^-3

P = 9.35×10^5 Pa

Partil pressure of oxygen will be -

P(O2) = P × n(O2) / n

P(O2) = 9.35×10^5 × 0.25 / 1.875

P(O2) = 1.24×10^5 Pa

Thanks dear...

Answer 2

Answer:

9.24

Explanation:

• answer ok